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Calculate the kinetic energy of an electron ejected by a photon with wavelength 1.91 x10^2 nm from a metal with a binding energy of 3.47 eV.
A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740.0 torr and a temperature of 25.0°C.
A mixture of gases conssists of CH4 at a partial pressure of 143 mm Hg, N2 at a partial pressure of 469 mm Hg, and O2 at a partial pressure of 563 mm Hg
If one started will 6.73 g of copper chloride, how many grams of copper could be produced?
How many moles of CO2 will be produced if 3.119 g of O2 are reacted completely?
if the freezing point of a .106 m CH3COOH solution is -.288 degrees celsius, calculate the percent of the acid that has undergone ionization?
calculate the amount of heat transfered when 24.0 g of CH3OH decompose at constant pressure. delta H is 126.4 kJ
When the sodium atom becomes a sodium ion, how does the size and electron configuration of the sodium atom change?
Explain the fact that even though dibenzoylmethane is not a methyl ketone it gives a positive iodoform test
A diprotic acid, H2A, has pKs 8.4 and 3.5. 50.0 mL of 0.10M of the diprotic acid, H2A, is titrated with 0.20 M NaOH. What is the Ve (i.e. the first equivalence point)?
Assuming the solution has a heat capacity of 4.18 J/°Cg and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol."
If B gas at 0.221 bar is injected into a container at 665 °C that contains excess A, what are the partial pressures of all gases present at equilibrium?
What mass of CCl2F2 substance must evaporate in order to freeze 109 of water initially at 24 degrees celsius? (The heat of fusion of water is 334 J/g the specific heat of water is 4.18 J/gK .)
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